What is the empirical formula of a compound containing #C, H#, and #O# if combustion of 3.69 g of the compound yields 5.40 g of #CO_2# and 2.22 g of #H_2O#?
We get finally an empirical formula of
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To determine the empirical formula of the compound, we need to find the moles of carbon, hydrogen, and oxygen in the compound.
Given: Mass of CO2 produced = 5.40 g Mass of H2O produced = 2.22 g
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Calculate the moles of carbon in CO2: Molar mass of CO2 = 12.01 g/mol (C) + 2(16.00 g/mol) (O) = 44.01 g/mol Moles of carbon = Mass of CO2 / Molar mass of CO2 = 5.40 g / 44.01 g/mol = 0.1227 mol
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Calculate the moles of hydrogen in H2O: Molar mass of H2O = 2(1.01 g/mol) (H) + 16.00 g/mol (O) = 18.02 g/mol Moles of hydrogen = Mass of H2O / Molar mass of H2O = 2.22 g / 18.02 g/mol = 0.1232 mol
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Determine the moles of oxygen: The moles of oxygen can be found by subtracting the sum of moles of carbon and hydrogen from the total moles of CO2 and H2O. Total moles of CO2 and H2O = 0.1227 mol (C) + 0.1232 mol (H) = 0.2459 mol Moles of oxygen = Total moles of CO2 and H2O - (moles of carbon + moles of hydrogen) = 0.2459 mol - (0.1227 mol + 0.1232 mol) = 0.0000 mol
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Determine the ratio of moles of each element to the smallest number of moles: Since the moles of oxygen are negligible, we consider the moles of carbon and hydrogen. The smallest number of moles is 0.1227 mol. So, the ratio of moles of carbon to the smallest number of moles is 1, and the ratio of moles of hydrogen to the smallest number of moles is approximately 1.
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Write the empirical formula: The empirical formula is CH.
Therefore, the empirical formula of the compound containing C, H, and O is CH.
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When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
When evaluating a one-sided limit, you need to be careful when a quantity is approaching zero since its sign is different depending on which way it is approaching zero from. Let us look at some examples.
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